Calculate the volume of a 1.16 M sulfuric acid (H2SO4) solution containing 0.116 mol of solute.
Given:
M = 1.16 M
number of mol = 0.116 mol
use:
M = number of mol / volume in L
1.16 = 0.116/ volume in L
volume = 0.100 L
volume = 100 mL
Answer: 100 mL
Calculate the volume of a 1.16 M sulfuric acid (H2SO4) solution containing 0.116 mol of solute.
a sulfuric acid solution containing 551.5 (a) A sulfuric acid solution containing 551.5g of H2SO4 per liter of Solution has a density of 1-339 Icme. Calculate molality of HaSO4 in this solution. the
Calculate the volume of a 0.150 M KCl solution containing 6.00 x 10-2 mol of solute. Enter your answer in the provided box. L Calculate the number of mol of solute in 3.00 x 102 mL of 0.500 M HCI. Enter your answer in the provided box. mol HCI mol HCI
Calculate the number of moles of solute in 2.00 L of 15.0 M H2SO4, concentrated sulfuric acid.
Two aqueous sulfuric acid (H2SO4) solutions containing 20.0 wt% H2SO4 (SG=1.139) and 80.0 wt% H2SO4 (SG=1.727) respectively, are mixed to form a 4.00 molar solution (mol/L) (SG=1.213). Calculate the mass fraction of sulfuric acid in the product stream. Atomic weight: H=1g/mol, O=16g/mol, S=32g/mol. Taking 100 kg of the 20 wt% feed solution as a basis, calculate the volumetric feed ratio of 20.0 wt% H2SO4 to 80.0 wt% H2SO4, to 2 decimal places.
Calculate the molality of a 35.0% (by mass) aqueous solution of sulfuric acid (H2SO4). (Molar mass of H2SO4 is 98.02 g/mol and for H2O is 18.02 g/mol) O 19.4 m 2.19 m W O 5.49 m O 3.57 m O 6.64 m
A sulfuric acid solution containing 571.6 g of H2SO4 per liter of solution has a density of 1.329 g/cm3. Calculate the following quantities for the solute in this solution. 9 pts 1. i. Mass percent ii. Molality iii. Molarity Table 1. Reference data Density @ Vapor Normal 20°C Pressure (torr) H20 1.86 0.00 0.512 100.00 0.998 17.5 2.53 80.1 0.8765 98.5 Normal point (oC) lKb value) boiling! (PC/m) point (C) Substance Formula Formula Kr value* Krvalue -20°C (°C/m) freezingb (g/mL)...
Calculate the molality of a 35.0% (by mass) aqueous solution of sulfuric acid (H2SO4). (Molar mass of H2SO4 is 98.02 g/mol and for H2O is 18.02 g/mol)
A solution is prepared containing 2.452g of sulfuric acid and 3.551g of sodium sulfate in a total volume of 500. mL. What are the molar concentrations of each solute in this solution?
To carry out a reaction, 20 mL of a solution of sulfuric acid (H2SO4) having a density of 1.84 g / mL and 85% by weight of the solute was used. Calculate the grams of H2SO4 that were used.
Calculate the concentrations of H2SO4, HSO4−, SO42− and H3O+ ions in a 0.12 M sulfuric acid solution at 25°C (Ka2for sulfuric acid is 1.3 × 10−2.) a). H2SO4 b). HSO4- c). SO42- d). H3O+